Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter Teacher Notes and Answers Chapter 10 SECTION 1 3. a. Liquid molecules are very mobile. This mobility allows a liquid to take the shape of its container. In liquids, molecules are in contact with adjacent molecules, allowing intermolecular forces to have a greater effect than they do in gases. The molecules in a liquid will therefore not necessarily spread out to fill a container’s entire volume. b. Polar molecules are attracted to adjacent molecules and are therefore less able to escape from the liquid’s surface than are nonpolar molecules. 4. An attractive force pulls adjacent parts of a liquid’s surface together, thus decreasing surface area to the smallest possible size. A sphere offers the minimum surface area for a given volume of liquid. 5. Freezing is a physical change. The substance solidifying is changing its state, which is a physical change. It is still the same substance so it has not changed chemically. 6. Evaporation is a physical change because it involves a change of physical state. There is no change in the chemical makeup of the substance, which would be necessary for a chemical change. 7. Evaporation is a form of vaporization. It occurs only in nonboiling liquids when some liquid particles enter the gas state. Vaporization is a more general term that refers to either a liquid or a solid changing to a gas. SHORT ANSWER 1. a. ideal gas b. ideal gas c. real gas 2. a. The energy is transferred between them. b. Those with the lower molecule mass. 3. a. Gas molecules are in constant, rapid, random motion. b. As a gas is heated, each molecule’s speed increases; therefore, the molecules pass through the small hole more frequently. 4. a. b, d, c, a b. All gases at the same temperature have the same average kinetic energy. Therefore, heavier molecules have slower average speeds. Thus, the gases are ranked from heaviest to lightest in molar mass. 5. Polar molecules attract neighboring polar molecules and often move out of their straight-line paths because of these attractions. 6. c. 7. In both cases the average speed of the molecules is proportional to temperature. The distribution of molecules becomes broader as the temperature increases. This means that there are a greater number of molecules traveling within a greater range of higher speeds as the temperature increases. SECTION 3 SECTION 2 SHORT ANSWER 1. b c a d 2. some possible answers: ionic solid: MgO, CaO, KI, CuSO4 covalent network solid: graphite, silicon carbide covalent molecular solid: dry ice SHORT ANSWER 1. a 2. a. Intermolecular forces are between separate molecules; intramolecular forces are within individual molecules. b. intermolecular c. intramolecular d. intermolecular Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 1 States of Matter Name: ______________________________Class: _________________ Date: _________________ 3. 4. 5. 6. (CO2), sulfur, iodine metallic solid: any metal from the far left side of the periodic table Solid lead is denser than the liquid form. a. crystalline solid b. crystalline solid c. amorphous solid d. amorphous solid a. Metals have many electrons that are not bound to any one atom; therefore they are able to move throughout the crystal. In covalent network solids, all atoms (and electrons) are strongly bound in place and are not free to move. b. Solids have definite volume because their particles are packed very close together. There is very little empty space into which the particles can be compressed. Even at high temperatures their particles are held in relatively fixed positions. c. In amorphous solids, particles are arranged randomly; no specific amount of kinetic energy is needed to overcome the attractive forces holding the particles together. Thus, they do not have a point at which they melt, but melt over a range of temperatures. d. Ionic crystals have strong binding forces between the positive and negative ions in the crystal structure. Covalent molecular crystals have weaker bonds between the molecules. The attractive forces between CH4 molecules are weak (dispersion forces). Little energy is needed to separate the molecules. Melting water ice involves the breaking of many hydrogen bonds between molecules, which requires more energy. d b a 4. a. A b. C c. it decreases d. ice and liquid water will vaporize, forming water vapor 5. a. decrease b. reverse reaction c. forward reaction 6. a. about 75C b. about 85C c. about 38 kPa d. Based solely on molar mass, CCl4 would be expected to be less volatile than water. However, CCl4 is nonpolar and thus has weak intermolecular forces of attraction. Water is polar and contains strong hydrogen bonds between molecules. Thus, water is less volatile despite its smaller molar mass. SECTION 5 SHORT ANSWER 1. a. physical b. chemical c. chemical d. physical 2. a. water b. formaldehyde c. water d. water 3. Hydrogen bonding in water occurs between a hydrogen atom of one water molecule and the unshared pair of electrons of an oxygen atom of an adjacent water molecule. It is a particularly strong type of dipole-dipole force. Hydrogen bonding causes the boiling point of water and its molar enthalpy of vaporization to be relatively high. The water’s high surface tension is also a result of hydrogen bonding. 4. a. 68.6 kJ/mol b. 79.8 cal/g 5. a. 14.7 g b. 0.814 mol c. 4.89 kJ SECTION 4 SHORT ANSWER 1. a 2. b c a d 3. c Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 2 States of Matter Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. Identify whether the descriptions below describe an ideal gas or a real gas. __________________ a. The gas will not condense because the molecules do not attract each other. __________________ b. Collisions between molecules are perfectly elastic. __________________ c. Gas particles passing close to one another exert an attraction on each other. 1 2. The formula for kinetic energy is KE mv 2 . 2 a. As long as temperature is constant, what happens to the kinetic energy of the colliding particles during an elastic collision? _____________________________________________________________ b. If two gases have the same temperature and share the same energy but have different molecular masses, which molecules will have the greater speed? _____________________________________________________________ 3. Use the kinetic-molecular theory to explain each of the following phenomena: a. A strong-smelling gas released from a container in the middle of a room is soon detected in all areas of that room. _____________________________________________________________ b. As a gas is heated, its rate of effusion through a small hole increases if all other factors remain constant. _____________________________________________________________ _____________________________________________________________ 4. a. ________________ List the following gases in order of rate of effusion, from lowest to highest. (Assume all gases are at the same temperature and pressure.) (a) He (b) Xe (c) HCl (d) Cl2 Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 3 States of Matter Name: ______________________________Class: _________________ Date: _________________ SECTION 1 continued b. Explain why you put the gases in the order above. Refer to the kineticmolecular theory to support your explanation. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 5. Explain why polar gas molecules experience larger deviations from ideal behavior than nonpolar molecules when all other factors (mass, temperature, etc) are held constant. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 6. _____ The two gases in the figure below are simultaneously injected into opposite ends of the tube. The ends are then sealed. They should just begin to mix closest to which labeled point? 7. Explain the difference in the speed-distribution curves of a gas at the two temperatures shown in the figure below. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 4 States of Matter Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter SECTION 2 SHORT ANSWER Answer the following questions in the space provided. 1. _____ Liquids possess all the following properties except (a) relatively low density. (c) relative incompressibility. (b) the ability to diffuse. (d) the ability to change to a gas. 2. a. Chemists distinguish between intermolecular and intramolecular forces. Explain the difference between these two types of forces. _______________________________________________________________ _______________________________________________________________ Classify each of the following as intramolecular or intermolecular: __________________ b. hydrogen bonding in liquid water __________________ c. the OH covalent bond in methanol, CH3OH __________________ d. the bonds that cause gaseous Cl2 to become a liquid when cooled 3. Explain the following properties of liquids by describing what is occurring at the molecular level. a. A liquid takes the shape of its container but does not expand to fill its volume. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ b. Polar liquids are slower to evaporate than nonpolar liquids. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 5 States of Matter Name: ______________________________Class: _________________ Date: _________________ SECTION 2 continued 4. Explain briefly why liquids tend to form spherical droplets, decreasing surface area to the smallest size possible. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 5. Is freezing a chemical change or a physical change? Briefly explain your answer. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 6. Is evaporation a chemical or physical change? Briefly explain your answer. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 7. What is the relationship between vaporization and evaporation? _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 6 States of Matter Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter SECTION 3 SHORT ANSWER Answer the following questions in the space provided. 1. Match description on the right to the correct crystal type on the left. ______ ionic crystal (a) has mobile electrons in the crystal ______ covalent molecular crystal (b) is hard, brittle, and nonconducting ______ metallic crystal (c) typically has the lowest melting point of the four crystal types ______ covalent network crystal (d) has strong covalent bonds between neighboring atoms 2. For each of the four types of solids, give a specific example other than one listed in the text. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 3. A chunk of solid lead is dropped into a pool of molten lead. The chunk sinks to the bottom of the pool. What does this tell you about the density of the solid lead compared with the density of the molten lead? _______________________________________________________________ 4. Answer amorphous solid or crystalline solid to the following questions: __________________ a. Which is less compressible? __________________ b. Which has a more clearly defined shape? __________________ c. Which is sometimes described as a supercooled liquid? __________________ d. Which has a less clearly defined melting point? Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 7 States of Matter Name: ______________________________Class: _________________ Date: _________________ SECTION 3 continued 5. Explain the following properties of solids by describing what is occurring at the atomic level. a. Metallic solids conduct electricity well, but covalent network solids do not. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ b. The volume of a solid changes only slightly with a change in temperature or pressure. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ c. Amorphous solids do not have a definite melting point. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ d. Ionic crystals are much more brittle than covalent molecular crystals. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ 6. Experiments show that it takes 6.0 kJ of energy to melt 1 mol of water ice at its melting point but only about 1.1 kJ to melt 1 mol of methane, CH4, at its melting point. Explain in terms of intermolecular forces why it takes so much less energy to melt the methane. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 8 States of Matter Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter SECTION 4 SHORT ANSWER Answer the following questions in the space provided. 1. _____ When a substance in a closed system undergoes a phase change and the system reaches equilibrium, (a) the two opposing changes occur at equal rates. (b) there are no more phase changes. (c) one phase change predominates. (d) the amount of substance in the two phases changes. 2. Match the following definitions on the right with the words on the left. ______ Equilibrium (a) melting ______ volatile (b) opposing changes occurring at equal rates in a closed system (c) readily evaporated ______ fusion ______ deposition (d) a change directly from a gas to a solid 3. Match the process on the right with the change of state on the left. ______ solid to gas (a) melting ______ liquid to gas (b) condensation ______ gas to liquid (c) sublimation ______ solid to liquid (d) vaporization 4. Refer to the phase diagram for water in Figure 16 on page 347 of the text to answer the following questions: __________________ a. What point represents the conditions under which all three phases can coexist? __________________ b. What point represents a temperature above which only the vapor phase exists? __________________ c. Based on the diagram, as the pressure on the water system increases, what happens to the melting point of ice? d. What happens when water is at point A on the curve and the temperature increases while the pressure is held constant? _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 9 States of Matter Name: ______________________________Class: _________________ Date: _________________ SECTION 4 continued 5. Use this general equilibrium equation to answer the following questions: reactants products energy __________________ a. If the forward reaction is favored, will the concentration of reactants increase, decrease, or stay the same? __________________ b. If extra product is introduced, which reaction will be favored? __________________ c. If the temperature of the system decreases, which reaction will be favored? 6.Refer to the graph below to answer the following questions: __________________ a. What is the normal boiling point of CCl4? __________________ b. What would be the boiling point of water if the air pressure over the liquid were reduced to 60 kPa? __________________ c. What must the air pressure over CCl4 be for it to boil at 50C? d. Although water has a lower molar mass than CCl4, it has a lower vapor pressure when measured at the same temperature. What makes water vapor less volatile than CCl4? _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 10 States of Matter Name: ______________________________Class: _________________ Date: _________________ CHAPTER 10 REVIEW States of Matter SECTION 5 SHORT ANSWER Answer the following questions in the space provided. 1. Indicate whether each of the following is a physical or chemical property of water. __________________ a. The density of ice is less than the density of liquid water. __________________ b. A water molecule contains one atom of oxygen and two atoms of hydrogen. __________________ c. There are strong hydrogen bonds between water molecules. __________________ d. Ice consists of water molecules in a hexagonal arrangement. 2. Compare a polar water molecule with a less-polar molecule, such as formaldehyde, CH2O. Both are liquids at room temperature and 1 atm pressure. __________________ a. Which liquid should have the higher boiling point? __________________ b. Which liquid is more volatile? __________________ c. Which liquid has a higher surface tension? __________________ d. In which liquid is NaCl, an ionic crystal, likely to be more soluble? 3. Describe hydrogen bonding as it occurs in water in terms of the location of the bond, the particles involved, the strength of the bond, and the effects this type of bonding has on physical properties. _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ _______________________________________________________________ Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 11 States of Matter Name: ______________________________Class: _________________ Date: _________________ SECTION 5 continued PROBLEMS Write the answer on the line to the left. Show all your work in the space provided. 4. The molar enthalpy of vaporization of water is 40.79 kJ/mol, and the molar enthalpy of fusion of ice is 6.009 kJ/mol. The molar mass of water is 18.02 g/mol. __________________ a. How much energy is absorbed when 30.3 g of liquid water boils? __________________ b. An energy unit often encountered is the calorie (4.18 J = 1 calorie). Determine the molar enthalpy of fusion of ice in calories per gram. 5. A typical ice cube has a volume of about 16.0 cm3 . Calculate the amount of energy needed to melt the ice cube. (Density of ice at 0.C = 0.917 g/mL; molar enthalpy of fusion of ice = 6.009 kJ/mol; molar mass of H2O = 18.02 g/mol.) __________________ a. Determine the mass of the ice cube. __________________ b. Determine the number of moles of H2O present in the sample. __________________ c. Determine the number of kilojoules of energy needed to melt the ice cube. Original content Copyright © by Holt, Rinehart and Winston. Additions and changes to the original content are the responsibility of the instructor. Modern Chemistry 12 States of Matter